Question

Identify the following properties as more typical of organic or inorganic compounds: a. contains \(\mathrm{Na}\) and \(\mathrm{Br}\) \(\mathbf{b}\). is a gas at room temperature c. contains covalent bonds d. is an electrolyte

Short answer

a. Inorganic, b. Organic, c. Organic, d. Inorganic

Step-by-step solution

- Identify the typical elements

Elements like \(\text{Na}\) and \(\text{Br}\) are typical of inorganic compounds. Organic compounds primarily contain \(\text{C}\) and \(\text{H}\).

- State of matter at room temperature

Gases at room temperature can be both organic (like methane, \(\text{CH}_4\)) and inorganic (like nitrogen, \(\text{N}_2\)). However, in the context of typical properties, organic compounds such as hydrocarbons (e.g., methane) are often gases due to their volatility.

- Types of bonds

Covalent bonds are more typical of organic compounds as they primarily involve the sharing of electrons between \(\text{C}\) and \(\text{H}\) atoms, whereas inorganic compounds often involve ionic bonds.

- Electrolyte behavior

Electrolytes are typically inorganic compounds because they dissociate into ions in solution, allowing them to conduct electricity. Organic compounds generally do not dissociate fully and are poor electrolytes.

Key concepts

Covalent Bonds

A covalent bond is a type of chemical bond where atoms share pairs of electrons. This allows each atom to attain the electron configuration of a noble gas. Covalent bonds are more common in organic compounds, which are compounds mainly composed of carbon and hydrogen.
In organic chemistry, carbon atoms often form covalent bonds with other elements, primarily hydrogen, oxygen, and nitrogen. This sharing of electrons can result in the formation of single, double, or even triple bonds.
Consider the molecule methane \(CH_4\). Here, carbon shares electrons with four hydrogen atoms through single covalent bonds. This structure is very stable and makes up the backbone of many organic compounds.
Covalent bonds can also be found in inorganic compounds, but they predominate in organic chemistry. This is because carbon has four valence electrons and can form multiple stable covalent bonds, leading to a vast array of organic molecules.

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water and can conduct electricity. This is a typical property of inorganic compounds. Common electrolytes include salts like sodium chloride (\(NaCl\)) and potassium bromide (\(KBr\)). When these substances dissolve in water, they break apart into their respective ions (e.g., \[Na^+\] and \[Cl^-\]).
In contrast, most organic compounds do not typically act as electrolytes. Organic molecules like glucose (\(C_6H_{12}O_6\)) dissolve in water but do not dissociate into ions. As a result, they do not conduct electricity.
This behavior is particularly important in biological systems where electrolytes help regulate nerve and muscle function, hydrate the body, balance blood acidity and pressure, and help rebuild damaged tissue. Hence, electrolytes are key to many physiological processes.

States of Matter

The state of matter refers to the physical form that a substance takes at room temperature: solid, liquid, or gas. This property can often hint at whether a compound is organic or inorganic.
Many organic compounds, especially volatile ones like methane (\(CH_4\)), can exist as gases at room temperature. This is because organic molecules may not have strong intermolecular forces compared to ionic compounds.
Inorganic compounds, on the other hand, are often solids at room temperature. For example, sodium chloride (table salt, \(NaCl\)) is a solid, as is potassium iodide (\(KI\)). This is due to the strong ionic bonds that hold their ions together in a regular lattice structure.
The understanding of the states of matter is crucial, not just for identifying compounds, but also in practical applications like gas laws, solution chemistry, and when dealing with reactions in different states.